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Margaret [11]
3 years ago
15

An ice cute at 0.0*C was dropped into 30.0 g of water in a

Chemistry
1 answer:
PilotLPTM [1.2K]3 years ago
5 0

<u>Answer:</u> The mass of ice cube is 77.90 grams

<u>Explanation:</u>

When ice is mixed with water, the amount of heat released by ice will be equal to the amount of heat absorbed by water.

Heat_{\text{absorbed}}=Heat_{\text{released}}

The equation used to calculate heat released or absorbed follows:

Q=m\times c\times \Delta T=m\times c\times (T_{final}-T_{initial})

m_1\times c_1\times (T_{final}-T_1)=-[m_2\times c_2\times (T_{final}-T_2)]       ......(1)

where,

m_1 = mass of ice = ? g

m_2 = mass of water = 30.0 g

T_{final} = final temperature = 19.5°C

T_1 = initial temperature of ice = 0.0°C

T_2 = initial temperature of water = 45.0°C

c_1 = specific heat of ice = 2.108  J/g°C

c_2 = specific heat of water = 4.186 J/g°C

Putting values in equation 1, we get:

m_1\times 2.108\times (19.5-0)=-[30.0\times 4.186\times (19.5-45.0)]

m_1=77.90g

Hence, the mass of ice cube is 77.90 grams

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A mixture of 15.0 g of the anesthetic halothane (C2HBrClF3 197.4 g/mol) and 22.6 g of oxygen gas has a total pressure of 862 tor
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Answer : The partial pressure of C_2HBrClF_3 and O_2 are, 84 torr and 778 torr respectively.

Explanation : Given,

Mass of C_2HBrClF_3 = 15.0 g

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Molar mass of C_2HBrClF_3 = 197.4 g/mole

Molar mass of O_2 = 32 g/mole

First we have to calculate the moles of C_2HBrClF_3 and O_2.

\text{Moles of }C_2HBrClF_3=\frac{\text{Mass of }C_2HBrClF_3}{\text{Molar mass of }C_2HBrClF_3}=\frac{15.0g}{197.4g/mole}=0.0759mole

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\text{Moles of }O_2=\frac{\text{Mass of }O_2}{\text{Molar mass of }O_2}=\frac{22.6g}{32g/mole}=0.706mole

Now we have to calculate the mole fraction of C_2HBrClF_3 and O_2.

\text{Mole fraction of }C_2HBrClF_3=\frac{\text{Moles of }C_2HBrClF_3}{\text{Moles of }C_2HBrClF_3+\text{Moles of }O_2}=\frac{0.0759}{0.0759+0.706}=0.0971

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\text{Mole fraction of }O_2=\frac{\text{Moles of }O_2}{\text{Moles of }C_2HBrClF_3+\text{Moles of }O_2}=\frac{0.706}{0.0759+0.706}=0.903

Now we have to partial pressure of C_2HBrClF_3 and O_2.

According to the Raoult's law,

p^o=X\times p_T

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p^o = partial pressure of gas

p_T = total pressure of gas

X = mole fraction of gas

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p_{O_2}=X_{O_2}\times p_T

p_{O_2}=0.903\times 862torr=778torr

Therefore, the partial pressure of C_2HBrClF_3 and O_2 are, 84 torr and 778 torr respectively.

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